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EC number: 231-302-2 | CAS number: 7488-55-3
- Life Cycle description
- Uses advised against
- Endpoint summary
- Appearance / physical state / colour
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- Endpoint summary
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- Ecotoxicological Summary
- Aquatic toxicity
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- Short-term toxicity to fish
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- Additional toxicological data

Hydrolysis
Administrative data
Link to relevant study record(s)
- Endpoint:
- hydrolysis
- Data waiving:
- study scientifically not necessary / other information available
- Justification for data waiving:
- other:
- Validity criteria fulfilled:
- yes
- Conclusions:
- Tin(II) can be hydrolysed into SnOH^{+}, Sn(OH)_{2} and Sn(OH)^{-}_{3}. In The pH frame according the guideline most of the Sn(II) exists as
Sn(OH)_{2}. The equilibrium constant for the dissioziation logK = 7.8 +/- 0.2 (@20°C).
Martyak reports for the hydrolysis reaction of stannos sulfate a free energy of %DELTA G = -7.37 kcal/mol and a equilibrium constant of ~1.8 x 10^5.
So the stannous sulfate ist not stable in water. Under alkaline conditions (pH>8 ) changes immediately oxidation state 2 to 4.
Reference
Sédy et al. pointed out that in the most studies to high concentrations of tin were used and so polytin complexes were formed. Further Sédy et al. show that there is a different in the species formed in a solution with and without halogeninde.
The values measured under standard conditions (25°C, 1bar)
Chemical equilibrium |
-log^{m}K° |
I (mol L^{-}) |
Remark |
Sn^{2+} + H_{2}O <=> SnOH^{+} + H^{+} |
3.8 +/- 0.2 |
0.1, 0.5, 1.0 |
Inorganic tin hydrolysis |
Sn^{2+} + 2H_{2}O <=> Sn(OH)^{0}_{2} + 2H^{+} |
7.8 +/- 0.2 |
0.1, 0.5, 1.0 |
Inorganic tin hydrolysis |
Sn^{2+} +3H_{2}O <=> SnOH^{-}_{3} + 3H^{+} |
-17.5 +/- 0.2 |
0.1, 0.5, 1.0 |
Inorganic tin hydrolysis |
Sn(OH)_{2}(s)óSn^{2+} + OH^{-} |
25.80 |
0_{corr} |
Precipitation Reactions |
SnO(s) + H_{2}O <=> Sn^{2+} + OH^{-} |
26.24 |
0_{corr} |
Precipitation Reactions |
The ion interaction coefficients are:
%epsilon |
Value (L mol^{-1} |
Sn^{2+}, NO_{3}^{-} |
0.4 +/- 0.1 |
SnOH^{+}, NO_{3}^{-} |
0.2 +/- 0.1 |
Sn(OH)_{2}, NO_{3}^{-} |
0.3 +/- 0.1 |
H^{+}, NO_{3}^{-} |
0.07 +/- 0.01 |
Distribution of various species of tin (II) as a function of pH
|
Sn^{2+} / % |
Sn(OH)^{+} / % |
Sn(OH)_{2} / % |
Sn(OH)_{3}^{-} / % |
4.0 |
30 |
40 |
30 |
0 |
4.5 |
7 |
34 |
59 |
0 |
5.0 |
2 |
11 |
87 |
0 |
5.5 |
0 |
4 |
96 |
0 |
6.0 |
0 |
2 |
98 |
0 |
6.5 |
0 |
1 |
99 |
0 |
7.0 |
0 |
0 |
100 |
0 |
7.5 |
0 |
0 |
99 |
1 |
8.0 |
0 |
0 |
98 |
2 |
8.5 |
0 |
0 |
95 |
5 |
9.0 |
0 |
0 |
80 |
20 |
9.5 |
0 |
0 |
50 |
50 |
10.0 |
0 |
0 |
30 |
70 |
Distribution of various species of tin (II) as a function of pH in present of 10^{-2} mol L^{-} [Cl^{-}]
|
Sn^{2+} / % |
SnCl^{+} / % |
SnCl_{2} / % |
Sn(OH)^{+} / % |
Sn(OH)_{2} / % |
Sn(OH)_{3}^{-} / % |
4.0 |
27 |
10 |
1 |
35 |
27 |
0 |
4.5 |
8 |
3 |
0 |
29 |
60 |
0 |
5.0 |
0 |
0 |
0 |
15 |
85 |
0 |
5.5 |
0 |
0 |
0 |
5 |
95 |
0 |
6.0 |
0 |
0 |
0 |
3 |
97 |
0 |
6.5 |
0 |
0 |
0 |
1 |
99 |
0 |
7.0 |
0 |
0 |
0 |
0 |
100 |
0 |
7.5 |
0 |
0 |
0 |
0 |
99 |
1 |
8.0 |
0 |
0 |
0 |
0 |
98 |
2 |
8.5 |
0 |
0 |
0 |
0 |
95 |
5 |
9.0 |
0 |
0 |
0 |
0 |
80 |
20 |
9.5 |
0 |
0 |
0 |
0 |
50 |
50 |
10.0 |
0 |
0 |
0 |
0 |
30 |
30 |
recovery of data: 95%
Martyak reports for the hydrolysis reaction of stannos sulfate a free energy of %DELTA G = -7.37 kcal/mol and a equilibrium constant of ~1.8 x 10^5.
Description of key information
There are no proprietary studies investigating the hydrolysis of the substance in aqueous media. The substance of interest is an inorganic element.
Typically salts (ionic bonding) are electrovalent substance. Electrovalent substances are made up of ions in the solid state. The oppositely charged ions are held together by strong electrostatic (coulombic) force of attraction. Due to these forces the ions cannot move. When these substances are dissolved in water, the ions free themselves from this binding. Thus the break up of an electrovalent compound into free mobile ions when dissolved in water or when melted, is called electrolytic dissociation. In the liquid state the ions become free and mobile. But the oppositely charged ions always remain in close proximity of each other.
SnSO4(s) ---> Sn2+(aq) + SO42- (aq). This is a 100% dissociation.
In addition this dissociation behaviour is depended from the solubulity of the substance and environmental conditions. Tin(II) can be hydrolysed into SnOH+, Sn(OH)2 and Sn(OH)3-, based on the conditions. At environmental relevant pH-values the Sn(OH)2 species is the predominant one (Séby, 2001). Consequently it is not technically possible to perform testing to measure simple dissociation events so testing is waived.
Key value for chemical safety assessment
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